Question 1

Which of the following atoms does not participate in hydrogen bonding?
A)S
B)O
C)F
D)N
E)H

Accepted Answer

Hydrogen bonding occurs between hydrogen and highly electronegative atoms such as O, N, or F. Sulfur (S) is not highly electronegative and does not participate in hydrogen bonding.

Question 2

Which are considered van der Waals forces? I.dispersion forces
II)dipole-dipole interactions
III)hydrogen bonding
A)I and III
B)II only
C)III only
D)I,II,and III
E)I only

Accepted Answer

Van der Waals forces include dispersion forces (I) and dipole-dipole interactions (II). Hydrogen bonding (III) is often considered a special type of dipole-dipole interaction and is sometimes included under van der Waals forces.

Question 3

Which one of the following pure substance has both dispersion forces and dipole-dipole forces? A)HCl B)BCl₃ C)Br₂ D)H₂ E)CO₂

Accepted Answer

HCl is a polar molecule due to the difference in electronegativity between hydrogen and chlorine, which creates a dipole moment. This allows for dipole-dipole interactions. Additionally, all molecules exhibit dispersion forces (also known as London dispersion forces), including HCl.

Question 4

Which one of the following pure substances will exhibit hydrogen bonding? A)CH₄ B)H₂C=CH₂ C)H₂O D)CHCl₃ E)CHF₃

Accepted Answer

A substance exhibits hydrogen bonding if it contains at least one of the following elements: nitrogen, oxygen, or fluorine. Option C contains oxygen and therefore is capable of exhibiting hydrogen bonding. The other options do not contain any of these elements and are therefore not capable of exhibiting hydrogen bonding.

Question 5

The strongest intermolecular interactions between pentane (C₅H₁₂)molecules arise from A)dipole-dipole forces. B)London dispersion forces. C)hydrogen bonding. D)ion-dipole interactions. E)carbon-carbon bonds.

Accepted Answer

Pentane is a nonpolar molecule and does not have hydrogen bond donors or acceptors. Therefore, the strongest intermolecular interactions between pentane molecules arise from London dispersion forces, which are the result of temporary dipoles generated by the constantly fluctuating electron cloud around each molecule.

Question 6

Which substance will exhibit hydrogen bonding between molecules? A)(CH₃)₃N B)CH₃-O-CH₃ C)CH₃CH₂-OH D)CH₃CH₂-F E)HI

Accepted Answer

CH3CH2OH has a polar O-H bond, which can form hydrogen bonds with other polar molecules. A and D do not have hydrogen bonding due to the absence of hydrogen bonding acceptor (N, F are not bonded with H). B does not have polar groups to form hydrogen bonding. E, HI is a single molecule, not capable of exhibiting hydrogen bonding between molecules.

Question 7

Helium atoms do not combine to form He₂ molecules,yet He atoms do attract one another weakly through A)dipole-dipole forces. B)ion-dipole forces. C)dispersion forces. D)dipole-induced dipole forces. E)hydrogen bonding.

Accepted Answer

Helium is a noble gas that exists as a monatomic gas. Since it is a nonpolar molecule, it cannot participate in dipole-dipole or ion-dipole forces. However, it does experience weak attractive forces known as dispersion forces or London forces. These forces arise from temporary dipoles that occur due to the uneven distribution of electrons around the nucleus. As a result, there is a transient dipole moment that causes a weak attraction between neighboring helium atoms.

Question 8

In which of the following compounds will the molecules not form hydrogen bonds with each other?
A) 
B) 
C) 
D) 
E)

Accepted Answer

The answer of In which of the following compounds will...

Question 9

Which substance should exhibit hydrogen bonding in the liquid phase? A)PH₃ B)He C)H₂S D)CH₄ E)CH₃OH

Accepted Answer

Hydrogen bonding occurs between a hydrogen atom and a highly electronegative atom such as oxygen or nitrogen. The molecule CH3OH (methanol) has a hydroxyl (-OH) group, which can participate in hydrogen bonding in the liquid phase. Therefore, E is the best choice.

Question 10

Which of the following is defined as the attractive forces between polar molecules? I.dispersion forces
II)dipole-dipole interactions
III)ion-dipole interactions
A)I and III
B)II only
C)III only
D)I,II,and III
E)I only

Accepted Answer

Dipole-dipole interactions are defined as the attractive forces between polar molecules. Dispersion forces are attractive forces between nonpolar molecules or atoms, and ion-dipole interactions are attractive forces between an ion and a polar molecule. Therefore, only option II, dipole-dipole interactions, fits the definition given in the question.

Question 11

The strongest intermolecular interactions between hydrogen fluoride (HF)molecules arise from
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)ion-dipole interactions.
E)ionic bonds.

Accepted Answer

Hydrogen fluoride (HF) molecules can form hydrogen bonds, which are the strongest type of intermolecular forces. In a hydrogen bond, a hydrogen atom that is covalently bonded to a highly electronegative atom (such as fluorine) is attracted to a lone pair of electrons on another highly electronegative atom (such as fluorine) in a nearby HF molecule. This results in a very strong attraction between the molecules. Dipole-dipole forces and London dispersion forces are much weaker than hydrogen bonds. Ion-dipole interactions and ionic bonds involve the attraction between ions and polar molecules, and are not applicable to HF molecules, which are nonpolar.

Question 12

What is the name given to the attractive forces that hold particles together in the condensed phase?
A)ionic bonds
B)covalent bonds
C)intermolecular forces
D)electronegativity
E)electron attraction

Accepted Answer

The name given to the attractive forces that hold particles together in the condensed phase (solid and liquid) is intermolecular forces. Ionic and covalent bonds hold particles together in the solid state, but they are not considered intermolecular forces because they involve the transfer or sharing of electrons between atoms, while intermolecular forces involve the attraction between molecules or atoms in close proximity. Electronegativity and electron attraction are related concepts but are not specific enough to describe the forces holding particles together in the condensed phase.

Question 13

The strongest intermolecular interactions between ethyl alcohol (CH₃CH₂OH)molecules arise from A)dipole-dipole forces. B)London dispersion forces. C)hydrogen bonding. D)ion-dipole interactions. E)carbon-oxygen bonds.

Accepted Answer

The strongest intermolecular interactions between ethyl alcohol molecules arise from hydrogen bonding, which involves the attraction between the hydrogen atom of one molecule and the oxygen atom of another molecule. This type of interaction is stronger than dipole-dipole forces, London dispersion forces, ion-dipole interactions, or carbon-oxygen bonds.

Question 14

Which of the responses includes all of the following that can form hydrogen bonds with water molecules? I.Na⁺,II.CH₃COOH,III.C₂H₆,IV.CH₃NH₂ A)I and II B)I and III C)II and III D)II and IV E)III and IV

Accepted Answer

Only molecules that have polar covalent bonds and contain electronegative atoms (such as oxygen or nitrogen) can form hydrogen bonds with water molecules. Choice II and IV contain nitrogen in the form of amide groups (NH) which can form hydrogen bonds with water molecules. Therefore, the answer is Choice D, which contains both II and IV.

Question 15

In a sample of hydrogen iodide,__________________ are the most important intermolecular forces.
A)dipole-dipole forces
B)London dispersion forces
C)hydrogen bonding
D)covalent bonds
E)polar covalent bonds

Accepted Answer

The answer of In a sample of hydrogen iodide,__________________ are...

Question 16

What types of intermolecular forces exist between hydrogen fluoride molecules? I.London forces
II)dipole-dipole interactions
III)hydrogen bonding
IV)ion-dipole interactions
A)II and III
B)I,II,and III
C)I only
D)III only
E)I and III

Accepted Answer

Hydrogen fluoride (HF) molecules exhibit London dispersion forces (I), dipole-dipole interactions (II) due to the polar nature of HF, and hydrogen bonding (III) because hydrogen is directly bonded to fluorine, a highly electronegative atom.

Question 17

Which kinds of intermolecular forces exist between propane molecules? I.dispersion forces
II)dipole-dipole interactions
III)ion-dipole interactions
A)I only
B)II only
C)III only
D)I,II,and III
E)I and III

Accepted Answer

Propane molecules are nonpolar and do not have a permanent dipole moment, so there are no dipole-dipole or ion-dipole interactions. The only intermolecular force present between propane molecules is dispersion force, which is caused by temporary dipoles induced by the fluctuation of electrons in the molecules. Therefore, the correct choice is A) I only.

Question 18

Ammonia's unusually high melting point is the result of
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)covalent bonding.
E)ionic bonding.

Accepted Answer

Ammonia molecules can form hydrogen bonds with each other due to the presence of a lone pair of electrons on the nitrogen atom. These hydrogen bonds are relatively strong and require a significant amount of energy to break, which is why ammonia has a higher melting point compared to other similar molecules that cannot form hydrogen bonds.

Question 19

What is another name given to dispersion forces?
A)ion-dipole interactions
B)dipole-dipole interactions
C)hydrogen bonding
D)covalent forces
E)London forces

Accepted Answer

Dispersion forces are commonly referred to as London forces, named after the scientist Fritz London who first described them.

Question 20

The strongest intermolecular interactions between hydrogen sulfide (H₂S)molecules arise from A)dipole-dipole forces. B)London dispersion forces. C)hydrogen bonding. D)ion-dipole interactions. E)disulfide linkages.

Accepted Answer

Hydrogen sulfide (H2S) molecules exhibit dipole-dipole interactions due to the difference in electronegativity between hydrogen and sulfur, creating a polar molecule. However, H2S does not engage in hydrogen bonding to a significant extent because sulfur is not as electronegative as nitrogen, oxygen, or fluorine, which are typically involved in hydrogen bonds.

Quiz 11: Intermolecular Forces and the Physical Properties of Liquids and Solids

Which of the following atoms does not participate in hydrogen bonding?

Which are considered van der Waals forces? I.dispersion forces II) dipole-dipole interactions III) hydrogen bonding

Which one of the following pure substance has both dispersion forces and dipole-dipole forces?

Which one of the following pure substances will exhibit hydrogen bonding?

The strongest intermolecular interactions between pentane (C₅H₁₂) molecules arise from

Which substance will exhibit hydrogen bonding between molecules?

Helium atoms do not combine to form He₂ molecules,yet He atoms do attract one another weakly through

In which of the following compounds will the molecules not form hydrogen bonds with each other?

Which substance should exhibit hydrogen bonding in the liquid phase?

Which of the following is defined as the attractive forces between polar molecules? I.dispersion forces II) dipole-dipole interactions III) ion-dipole interactions

The strongest intermolecular interactions between hydrogen fluoride (HF) molecules arise from

What is the name given to the attractive forces that hold particles together in the condensed phase?

The strongest intermolecular interactions between ethyl alcohol (CH₃CH₂OH) molecules arise from

Which of the responses includes all of the following that can form hydrogen bonds with water molecules? I.Na⁺,II.CH₃COOH,III.C₂H₆,IV.CH₃NH₂

In a sample of hydrogen iodide,__________________ are the most important intermolecular forces.

What types of intermolecular forces exist between hydrogen fluoride molecules? I.London forces II) dipole-dipole interactions III) hydrogen bonding IV) ion-dipole interactions

Which kinds of intermolecular forces exist between propane molecules? I.dispersion forces II) dipole-dipole interactions III) ion-dipole interactions

Ammonia's unusually high melting point is the result of

What is another name given to dispersion forces?

The strongest intermolecular interactions between hydrogen sulfide (H₂S) molecules arise from